Domanda del libro di testo
(b) It turns out that ozone, O3, has a small dipole moment. How is this possible, given that all the atoms are the same?
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Ch.9 - Molecular Geometry and Bonding Theories
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Capitolo 9, Problema 39b
(b) If you react BF3 to make the ion BF32-, is this ion planar?
Guida verificata passo dopo passo1
Identify the central atom in the molecule BF3, which is boron (B).
Determine the electron configuration of boron. Boron has an atomic number of 5, so its electron configuration is 1s² 2s² 2p¹.
Understand the geometry of BF3. In BF3, boron forms three bonds with fluorine atoms, resulting in a trigonal planar shape due to sp² hybridization.
Consider the addition of two electrons to form BF3²⁻. Adding two electrons to the molecule will affect the electron geometry and hybridization.
Analyze the new geometry. With the addition of two electrons, the central boron atom will have a total of five electron pairs (three bonding pairs and two lone pairs), leading to a trigonal bipyramidal electron geometry. However, the presence of lone pairs will affect the molecular shape, making it non-planar.
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Molecular Geometry
Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. It is determined by the number of bonding pairs and lone pairs of electrons around the central atom, which influences the shape of the molecule. Understanding molecular geometry is crucial for predicting the spatial orientation of molecules and their reactivity.
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01:33
Molecular Geometry with Two Electron Groups
Hybridization
Hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals that can accommodate bonding. In the case of BF3, the boron atom undergoes sp2 hybridization, leading to a trigonal planar geometry. This concept helps explain the bonding and shape of molecules, which is essential for determining if a resulting ion like BF3^2- is planar.
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00:51Hybridization
Planarity in Ions
Planarity in ions refers to whether all atoms in the ion lie in the same geometric plane. For an ion to be planar, it typically must have a specific arrangement of bonds and electron pairs that allows for such a configuration. Analyzing the electron distribution and molecular geometry helps determine if the ion BF3^2- maintains a planar structure.
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02:07Square planar complexes show the most complex splitting pattern.
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Predict whether each of the following molecules is polar or nonpolar: (a) IF, (b) CS2, (c) SO3, (d) PCl3, (e) SF6, (f) IF5.
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Domanda del libro di testo
(a) Consider the following two molecules: PCl3 and BCl3. Which molecule has a nonzero dipole moment?
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Domanda del libro di testo
(c) Does the molecule BF2Cl have a dipole moment?
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Domanda del libro di testo
(a) Does CS2 have a dipole moment? If so, in which direction does the net dipole point? (b) Does SO2 have a dipole moment? If so, in which direction does the net dipole point?
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